Chemistry (entropy)

posted by .

Calculate the Ksp of CaF2 (2 is subscript).
The problem wants it calculated with all or one of the following:
G = -1162 kJ/mol
H = -1215 kJ/mol
S = 68.87 J/mol*k

The answer is 1.55*10^(-10). How do I do this?

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    Calculate S (measure of total entropy) for the following reaction at 25C and 1atm, and tell whether the entropy is increasing or decreasing. C3H8(g)+5O2(g)-> 3CO2(g)+4H2O(g) S of C3H8=64.5 cal/(mol*K) S of O2= 49 cal/(mol*K) S of …
  2. Chemistry Help!!!!

    Calculate S (measure of total entropy) for the following reaction at 25C and 1atm, and tell whether the entropy is increasing or decreasing. C3H8(g)+5O2(g)-> 3CO2(g)+4H2O(g) S of C3H8=64.5 cal/(mol*K) S of O2= 49 cal/(mol*K) S of …
  3. Chemistry

    Calculate S (measure of total entropy) for the following reaction at 25C and 1atm, and tell whether the entropy is increasing or decreasing. C3H8(g)+5O2(g)-> 3CO2(g)+4H2O(g) S of C3H8=64.5 cal/(mol*K) S of O2= 49 cal/(mol*K) S of …
  4. Chemistry 114

    Write down the Ksp expression for CaF2. If the molar solubility of CaF2 at 35℃ is 1.24×10^(-3)mol/dm3, calculate the value of Ksp.
  5. chemistry

    Which of the following mixtures will be a buffer when dissolved in a liter of water?
  6. CHEMISTRY

    Calculate ΔSfus and ΔSvap for HF. Determine the entropy change when 7.60 mol of HF(l) freezes at atmospheric pressure. I already calculated ΔSfus as 24.103 J/k*mol and ΔSvap as 86.07 J/K*mol....These are correct …
  7. CHEM

    Calculate ΔSfus and ΔSvap for HF. Determine the entropy change when 7.60 mol of HF(l) freezes at atmospheric pressure. I already calculated ΔSfus as 24.103 J/k*mol and ΔSvap as 86.07 J/K*mol....These are correct …
  8. chemistry

    Given a saturated solution of CaF2, write the ionic equilibrium and use it to calculate the solubility of CaF2. My answers for the ionic equation and ksp values are CaF2(s)<->Ca2+(aq)+ 2F-(aq) Ksp= [Ca2+][F-]2 ksp=2.02*10^-4 …
  9. Chemistry

    The standard entropy change for 1.00 moles of Ar as it evaporates at -185.7 °C (∆H°-185.7 = 1558 cal mol-1) is?
  10. Chemistry

    Calculate how many moles of Na2S2O3 must be added to dissolve 0.020 mol AgBr in 1.0 L of water at 25°C (assume constant volume). AgBr(s) ↔ Ag+(aq) + Br−(aq) Ksp = 3.3 x 10^−13 Ag+(aq) + 2S2O32−(aq) ↔ [Ag(S2O3)2]3−(aq) …

More Similar Questions